Download Chemistry Curriculum by Trimester

Whitman-Hanson Regional School District
Chemistry
Pacing Guide 2007-8
Trimester 1
Trimester 2
1. Properties of Matter
Central Concept: Physical and chemical properties
reflect the nature of the interactions between molecules
or atoms, and can be used to classify and describe
matter.
1.1 Identify and explain physical properties (e.g.,
density, melting point, boiling point,
conductivity, malleability) and chemical
properties (e.g., the ability to form new
substances). Distinguish between chemical
and physical changes.
1.2 Explain the difference between pure substances
(elements and compounds) and mixtures.
Differentiate between heterogeneous and
homogeneous mixtures.
1.3 Describe the three normal states of matter (solid,
liquid, gas) in terms of energy, particle
motion, and phase transitions.
2. Atomic Structure and Nuclear Chemistry
Central Concepts: Atomic models are used to explain
atoms and help us understand the interaction of elements
and compounds observed on a macroscopic scale.
Nuclear chemistry deals with radioactivity, nuclear
processes, and nuclear properties. Nuclear reactions
produce tremendous amounts of energy and lead to the
formation of elements.
2.1 Recognize discoveries from Dalton (atomic
theory), Thomson (the electron), Rutherford
(the nucleus), and Bohr (planetary model of
atom), and understand how each discovery
leads to modern theory.
2.2 Describe Rutherford’s “gold foil” experiment that
led to the discovery of the nuclear atom.
Identify the major components (protons,
neutrons, and electrons) of the nuclear atom
and explain how they interact.
2.3 Interpret and apply the laws of conservation of
mass, constant composition (definite
proportions), and multiple proportions.
5. Chemical Reactions and Stoichiometry
Central Concepts: In a chemical reaction, one or more
reactants are transformed into one or more new products.
Chemical equations represent the reaction and must be
balanced. The conservation of atoms in a chemical
reaction leads to the ability to calculate the amount of
products formed and reactants used (stoichiometry).
5.1 Balance chemical equations by applying the laws
of conservation of mass and constant
composition (definite proportions).
5.2 Classify chemical reactions as synthesis
(combination), decomposition, single
displacement (replacement), double
displacement, and combustion.
5.3 Use the mole concept to determine number of
particles and molar mass for elements and
compounds.
5.4 Determine percent compositions, empirical
formulas, and molecular formulas.
5.5 Calculate the mass-to-mass stoichiometry for a
chemical reaction.
5.6 Calculate percent yield in a chemical reaction.
6. States of Matter, Kinetic Molecular Theory, and
Thermochemistry
Central Concepts: Gas particles move independently of
each other and are far apart. The behavior of gas particles
can be modeled by the kinetic molecular theory. In
liquids and solids, unlike gases, particles are close to each
other. The driving forces of chemical reactions are energy
and entropy. The reorganization of atoms in chemical
reactions results in the release or absorption of heat
energy.
6.1 Using the kinetic molecular theory, explain the
behavior of gases and the relationship between
pressure and volume (Boyle’s law), volume
and temperature (Charles’s law), pressure and
temperature (Gay-Lussac’s law), and the
number of particles in a gas sample
(Avogadro’s hypothesis). Use the combined
2.4 Write the electron configurations for the first
twenty elements of the periodic table.
2.5 Identify the three main types of radioactive decay
(alpha, beta, and gamma) and compare their
properties (composition, mass, charge, and
penetrating power).
2.6 Describe the process of radioactive decay by
using nuclear equations, and explain the
concept of half-life for an isotope (for
example, C-14 is a powerful tool in
determining the age of objects).
2.7 Compare and contrast nuclear fission and nuclear
fusion.
3. Periodicity
Central Concepts: Repeating (periodic) patterns of
physical and chemical properties occur among elements
that define families with similar properties. The periodic
table displays the repeating patterns, which are related to
the atoms’ outermost electrons.
3.1 Explain the relationship of an element’s position
on the periodic table to its atomic number.
Identify families (groups) and periods on the
periodic table.
3.2 Use the periodic table to identify the three classes
of elements: metals, nonmetals, and
metalloids.
3.3 Relate the position of an element on the periodic
table to its electron configuration and compare
its reactivity to the reactivity of other elements
in the table.
3.4 Identify trends on the periodic table (ionization
energy, electronegativity, and relative sizes of
atoms and ions).
4. Chemical Bonding
Central Concept: Atoms bond with each other by
transferring or sharing valence electrons to form
compounds.
4.1 Explain how atoms combine to form compounds
through both ionic and covalent bonding.
Predict chemical formulas based on the
number of valence electrons.
4.2 Draw Lewis dot structures for simple molecules
and ionic compounds.
4.3 Use electronegativity to explain the difference
between polar and nonpolar covalent bonds.
4.4 Use valence-shell electron-pair repulsion theory
gas law to determine changes in pressure,
volume, and temperature.
6.2 Perform calculations using the ideal gas law.
Understand the molar volume at 273 K and 1
atmosphere (STP).
6.3 Using the kinetic molecular theory, describe and
contrast the properties of gases, liquids, and
solids. Explain, at the molecular level, the
behavior of matter as it undergoes phase
transitions.
6.4 Describe the law of conservation of energy.
Explain the difference between an
endothermic process and an exothermic
process.
6.5 Recognize that there is a natural tendency for
systems to move in a direction of disorder or
randomness (entropy).
7. Solutions, Rates of Reaction, and Equilibrium
Central Concepts: Solids, liquids, and gases dissolve to
form solutions. Rates of reaction and chemical
equilibrium are dynamic processes that are significant in
many systems (e.g., biological, ecological, geological).
7.1 Describe the process by which solutes dissolve in
solvents.
7.2 Calculate concentration in terms of molarity. Use
molarity to perform solution dilution and
solution stoichiometry.
7.3 Identify and explain the factors that affect the rate
of dissolving (e.g., temperature, concentration,
surface area, pressure, mixing).
7.4 Compare and contrast qualitatively the properties
of solutions and pure solvents (colligative
properties such as boiling point and freezing
point).
7.5 Identify the factors that affect the rate of a
chemical reaction (temperature, mixing,
concentration, particle size, surface area,
catalyst).
7.6 Predict the shift in equilibrium when a system is
subjected to a stress (LeChatelier’s principle)
and identify the factors that can cause a shift
in equilibrium (concentration, pressure,
volume, temperature).
8. Acids and Bases and Oxidation-Reduction
Reactions
Central Concepts: Acids and bases are important in
(VSEPR) to predict the molecular geometry
(linear, trigonal planar, and tetrahedral) of
simple molecules.
4.5 Identify how hydrogen bonding in water affects a
variety of physical, chemical, and biological
phenomena (e.g., surface tension, capillary
action, density, boiling point).
4.6 Name and write the chemical formulas for simple
ionic and molecular compounds, including
those that contain the polyatomic ions:
ammonium, carbonate, hydroxide, nitrate,
phosphate, and sulfate.
numerous chemical processes that occur around us, from
industrial procedures to biological ones, from the
laboratory to the environment. Oxidation-reduction
reactions occur when one substance transfers electrons to
another substance, and constitute a major class of
chemical reactions.
8.1 Define the Arrhenius theory of acids and bases in
terms of the presence of hydronium and
hydroxide ions in water and the BronstedLowry theory of acids and bases in terms of
proton donors and acceptors.
8.2 Relate hydrogen ion concentrations to the pH
scale and to acidic, basic, and neutral
solutions. Compare and contrast the strengths
of various common acids and bases (e.g.,
vinegar, baking soda, soap, citrus juice).
8.3 Explain how a buffer works.
8.4 Describe oxidation and reduction reactions and
give some everyday examples, such as fuel
burning and corrosion. Assign oxidation
numbers in a reaction.